Covalent Bonding Notes Ionic vs Covalent Bonding Ionic
![Covalent Bonding Notes Covalent Bonding Notes](https://slidetodoc.com/presentation_image/03b754fa143c92785712508606f8aa64/image-1.jpg)
Covalent Bonding Notes
![Ionic vs Covalent Bonding • Ionic: electron(s) leave one atom & gained by another Ionic vs Covalent Bonding • Ionic: electron(s) leave one atom & gained by another](http://slidetodoc.com/presentation_image/03b754fa143c92785712508606f8aa64/image-2.jpg)
Ionic vs Covalent Bonding • Ionic: electron(s) leave one atom & gained by another atom to satisfy both atoms’ octets, this results in the formation of ions. The resulting opposite charges attract each other. • Covalent: electrons are shared by two or more atoms to satisfy their octets.
![How can you tell if a bond is IONIC or COVALENT? • Subtract the How can you tell if a bond is IONIC or COVALENT? • Subtract the](http://slidetodoc.com/presentation_image/03b754fa143c92785712508606f8aa64/image-3.jpg)
How can you tell if a bond is IONIC or COVALENT? • Subtract the two electronegativity values (look at an electronegativity chart p. 263). >1. 7 to 4. 0: Ionic >0. 4 to 1. 7: Polar Covalent 0. 0 to 0. 4: Non-Polar Covalent • Electronegativity: atom’s ability to attract electrons in a chemical bond. (higher electronegativity means the atom wants electrons more)
![How can you tell if a bond is IONIC or COVALENT? • Easy way: How can you tell if a bond is IONIC or COVALENT? • Easy way:](http://slidetodoc.com/presentation_image/03b754fa143c92785712508606f8aa64/image-4.jpg)
How can you tell if a bond is IONIC or COVALENT? • Easy way: All metals = metallic bond Nonmetals and Metals = ionic bond All nonmetals = covalent bond
![Yes, there are 2 kinds of covalent bonds! • Polar covalent: the electrons are Yes, there are 2 kinds of covalent bonds! • Polar covalent: the electrons are](http://slidetodoc.com/presentation_image/03b754fa143c92785712508606f8aa64/image-5.jpg)
Yes, there are 2 kinds of covalent bonds! • Polar covalent: the electrons are shared, but one atom is pulling on the electrons a lot more. The electrons spend more time around that atom. • Nonpolar covalent: the electrons are evenly shared between the two atoms.
![O(3. 5) – H (2. 1) = 1. 4 Polar covalent bond O(3. 5) – H (2. 1) = 1. 4 Polar covalent bond](http://slidetodoc.com/presentation_image/03b754fa143c92785712508606f8aa64/image-6.jpg)
O(3. 5) – H (2. 1) = 1. 4 Polar covalent bond
![• The closer the elements are on the periodic table, their electronegativities are • The closer the elements are on the periodic table, their electronegativities are](http://slidetodoc.com/presentation_image/03b754fa143c92785712508606f8aa64/image-7.jpg)
• The closer the elements are on the periodic table, their electronegativities are more similar… more likely to form covalent bonds • Farther away… greater difference in electronegativity… more likely to form ionic bonds. • Metal + nonmetal = usually ionic • Nonmetal + nonmetal = usually covalent.
![Properties of Covalent Compounds 1) Covalent compounds generally have much lower melting and boiling Properties of Covalent Compounds 1) Covalent compounds generally have much lower melting and boiling](http://slidetodoc.com/presentation_image/03b754fa143c92785712508606f8aa64/image-8.jpg)
Properties of Covalent Compounds 1) Covalent compounds generally have much lower melting and boiling points than ionic compounds. 2) Covalent compounds are soft and squishy (compared to ionic compounds, anyway).
![Properties, Cont’d • 3) Covalent compounds tend to be more flammable than ionic compounds. Properties, Cont’d • 3) Covalent compounds tend to be more flammable than ionic compounds.](http://slidetodoc.com/presentation_image/03b754fa143c92785712508606f8aa64/image-9.jpg)
Properties, Cont’d • 3) Covalent compounds tend to be more flammable than ionic compounds. – There are exceptions to this rule! • 4) Covalent compounds don't conduct electricity in water.
![Bond Dissociation Energy • Bond dissociation energy = energy required to break a covalent Bond Dissociation Energy • Bond dissociation energy = energy required to break a covalent](http://slidetodoc.com/presentation_image/03b754fa143c92785712508606f8aa64/image-10.jpg)
Bond Dissociation Energy • Bond dissociation energy = energy required to break a covalent bond. Highest bond energy Hardest to break Triple Bond Shortest bond length Strongest Lowest bond energy Easiest to break Double Bond Single Bond Longest bond length Weakest
![How to Name Covalent Compounds • 1. Name the first element (normal name) • How to Name Covalent Compounds • 1. Name the first element (normal name) •](http://slidetodoc.com/presentation_image/03b754fa143c92785712508606f8aa64/image-11.jpg)
How to Name Covalent Compounds • 1. Name the first element (normal name) • 2. Name the second element (root name + “-ide”) • 3. Add prefixes to indicate how many atoms of each element are in the molecule (Subscripts) • Exception: no need to use “mono” for first element. Example: CO 2 = carbon dioxide
![Prefixes Subscript prefix 1 2 3 Mono Di. Tri- 4 5 6 7 8 Prefixes Subscript prefix 1 2 3 Mono Di. Tri- 4 5 6 7 8](http://slidetodoc.com/presentation_image/03b754fa143c92785712508606f8aa64/image-12.jpg)
Prefixes Subscript prefix 1 2 3 Mono Di. Tri- 4 5 6 7 8 9 10 Tetra. Penta. Hexa. Hepta. Octa. Nona. Deca-
![Memorize these exceptions Chemical formula name H 2 O water CH 4 Methane NH Memorize these exceptions Chemical formula name H 2 O water CH 4 Methane NH](http://slidetodoc.com/presentation_image/03b754fa143c92785712508606f8aa64/image-13.jpg)
Memorize these exceptions Chemical formula name H 2 O water CH 4 Methane NH 3 ammonia
![MEMORIZE THESE ACID NAMES Acid Name HCl Hydrochloric acid H 2 SO 4 Sulfuric MEMORIZE THESE ACID NAMES Acid Name HCl Hydrochloric acid H 2 SO 4 Sulfuric](http://slidetodoc.com/presentation_image/03b754fa143c92785712508606f8aa64/image-14.jpg)
MEMORIZE THESE ACID NAMES Acid Name HCl Hydrochloric acid H 2 SO 4 Sulfuric acid
![Diatomics • Diatomic elements are elements that do not exist singularly in nature because Diatomics • Diatomic elements are elements that do not exist singularly in nature because](http://slidetodoc.com/presentation_image/03b754fa143c92785712508606f8aa64/image-15.jpg)
Diatomics • Diatomic elements are elements that do not exist singularly in nature because they are highly reactive. “Which elements are the diatomics? ” “HON, it’s the halogens!” • H 2, O 2, N 2, F 2, Cl 2, Br 2, I 2
- Slides: 15